Metal Reactivity Series (D) Flashcards
List all the elements in the series from most reactive to least. (including carbon and hydrogen)
- Potassium
- Sodium
- Calcium
- Magnesium
- Aluminium
- Carbon
- Zinc
- Iron
- Tin
- Lead
- Hydrogen
- Copper
- Silver
- Gold
Please Stop Calling Me A Cute Zebra Instead Try Learning How Copper Saves Gold
Metal + Water → …
Metal Hydroxide + Hydrogen
Metal + Steam → …
Metal Oxide + Hydrogen
Why can’t carbon reduce metals potassium to magnesium from their oxides?
- Carbon is less reactive than these metals
- Carbon cannot displace and extract very reactive metals from their oxides
- Carbon cannot reduce the metal oxide to the metal
Why does some metal carbonates not decompose?
More reactive metals → More stable metal carbonates → More difficult to decompose the metal carbonate by heat.
State the effect of heating from Calcium to silver carbonates.
- Calcium to Copper (II) carbonates decompose into metal oxide and carbon dioxide.
- Silver Carbonate decompose into silver, oxygen and carbon dioxide easily.
Explain why Mg (s) displaces CuSO4 (aq).
- Magnesium is more reactive than copper.
- Magnesium displaces copper from copper(II) sulfate solution to form magnesium sulfate.
Describe the observation made from Mg (s) + CuSO4 (aq) → MgSO4 (aq) + CU (s)
- Copper(II) sulfate solution changes from blue to colourless (Magnesium sulfate solution is formed colourless)
- Reddish-brown solid is deposited (Copper)
Rusting can be sped up by…
- Dissolved Ionic Substances in water → increases conductivity and speed up rusting
- Presence of salt (Sodium Chloride), dilute acids (acid rain)
- Contact with another metal which is less reactive than iron. → Iron loses electrons to form Fe (2+) ions more readily than less reactive metals.
How does coating iron with plastic/oil/compound/less reactive metal prevent rust?
Serves as a barrier protection which prevents the contact of iron with oxygen and water
